Question 1

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)  MnO2(s) 
B)  Cl⁻(aq) 
C)  Ag⁺(aq) 
D)  SO42-(aq) 
E)  MnO4⁻(aq) 
A)  MnO2(s) 
B)  Cl⁻(aq) 
C)  Ag⁺(aq) 
D)  SO42-(aq) 
E)  MnO4⁻(aq)

Question 2

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s)+ 3 Mg2+(aq)→ 2 Al3+(aq)+ 3 Mg(s)

Accepted Answer

A)  +4.1 × 102 kJ 
B)  +1.4 × 102 kJ 
C)  -2.3 × 102 kJ 
D)  -7.8 × 102 kJ 
E)  +6.8 × 102 kJ 
A)  +4.1 × 102 kJ 
B)  +1.4 × 102 kJ 
C)  -2.3 × 102 kJ 
D)  -7.8 × 102 kJ 
E)  +6.8 × 102 kJ

Question 3

Identify the battery that is used as a common flashlight battery.

Accepted Answer

A)  dry-cell battery 
B)  lithium ion battery 
C)  lead-acid storage battery 
D)  NiCad battery 
E)  fuel cell 
A)  dry-cell battery 
B)  lithium ion battery 
C)  lead-acid storage battery 
D)  NiCad battery 
E)  fuel cell

Question 4

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. 4 F⁻(aq)+ Mn2+(aq)→ 2F2(g)+ Mn(s)
F2(g)+ 2e⁻ → 2 F⁻(aq)E° = +2.87 V
Mn2+(aq)+ 2 e⁻ → Mn(s)E° = -1.18 V

Accepted Answer

A)  1.69 V 
B)  4.05 V 
C)  -4.05 V 
D)  +2.87 V 
A)  1.69 V 
B)  4.05 V 
C)  -4.05 V 
D)  +2.87 V

Question 5

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Ag(s)+ Pb2+(aq)→ Ag+(aq)+ Pb(s)

Accepted Answer

A)  179 kJ 
B)  89.5 kJ 
C)  -328 kJ 
D)  -107 kJ 
E)  212 kJ 
A)  179 kJ 
B)  89.5 kJ 
C)  -328 kJ 
D)  -107 kJ 
E)  212 kJ

Question 6

How many kilowatt-hours of electricity are used to produce 3.50 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 4.50 V?

Accepted Answer

A)  0.0288 
B)  0.0347 
C)  8.7 
D)  34.7 
E)  17.4 
A)  0.0288 
B)  0.0347 
C)  8.7 
D)  34.7 
E)  17.4

Question 7

What is undergoing reduction in the redox reaction represented by the following cell notation?
Mn(s)∣ Mn2+(aq)   H+(aq)∣ H2(g)∣ Pt

Accepted Answer

A)  H2(g) 
B)  H+(aq) 
C)  Mn2+(aq) 
D)  Mn(s) 
E)  Pt 
A)  H2(g) 
B)  H+(aq) 
C)  Mn2+(aq) 
D)  Mn(s) 
E)  Pt

Question 8

Which of the following reactions would have the smallest value of K at 298 K?

Accepted Answer

A)  A + B → C; E°cell = +1.22 V 
B)  A + 2 B → C; E°cell = +0.98 V 
C)  A + B → 2 C; E°cell = -0.030 V 
D)  A + B → 3 C; E°cell = +0.15 V 
E)  More information is needed to determine. 
A)  A + B → C; E°cell = +1.22 V 
B)  A + 2 B → C; E°cell = +0.98 V 
C)  A + B → 2 C; E°cell = -0.030 V 
D)  A + B → 3 C; E°cell = +0.15 V 
E)  More information is needed to determine.

Which of the following is the strongest oxidizing agent?

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s)+ 3 Mg²⁺(aq)→ 2 Al³⁺(aq)+ 3 Mg(s)

Identify the battery that is used as a common flashlight battery.

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. 4 F⁻(aq)+ Mn²⁺(aq)→ 2F₂(g)+ Mn(s) F₂(g)+ 2e⁻ → 2 F⁻(aq)E° = +2.87 V Mn²⁺(aq)+ 2 e⁻ → Mn(s)E° = -1.18 V

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Ag(s)+ Pb²⁺(aq)→ Ag⁺(aq)+ Pb(s)

How many kilowatt-hours of electricity are used to produce 3.50 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 4.50 V?

What is undergoing reduction in the redox reaction represented by the following cell notation? Mn(s)∣ Mn²⁺(aq) H⁺(aq)∣ H₂(g)∣ Pt

Which of the following reactions would have the smallest value of K at 298 K?

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

Exam 20: Electrochemistry

Which of the following is the strongest oxidizing agent?

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s)+ 3 Mg2+(aq)→ 2 Al3+(aq)+ 3 Mg(s)

Identify the battery that is used as a common flashlight battery.

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. 4 F⁻(aq)+ Mn2+(aq)→ 2F2(g)+ Mn(s) F2(g)+ 2e⁻ → 2 F⁻(aq)E° = +2.87 V Mn2+(aq)+ 2 e⁻ → Mn(s)E° = -1.18 V

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Ag(s)+ Pb2+(aq)→ Ag+(aq)+ Pb(s)

How many kilowatt-hours of electricity are used to produce 3.50 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 4.50 V?

What is undergoing reduction in the redox reaction represented by the following cell notation? Mn(s)∣ Mn2+(aq) H+(aq)∣ H2(g)∣ Pt

Which of the following reactions would have the smallest value of K at 298 K?

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s)+ 3 Mg²⁺(aq)→ 2 Al³⁺(aq)+ 3 Mg(s)

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. 4 F⁻(aq)+ Mn²⁺(aq)→ 2F₂(g)+ Mn(s) F₂(g)+ 2e⁻ → 2 F⁻(aq)E° = +2.87 V Mn²⁺(aq)+ 2 e⁻ → Mn(s)E° = -1.18 V

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Ag(s)+ Pb²⁺(aq)→ Ag⁺(aq)+ Pb(s)

How many kilowatt-hours of electricity are used to produce 3.50 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 4.50 V?

What is undergoing reduction in the redox reaction represented by the following cell notation? Mn(s)∣ Mn²⁺(aq) H⁺(aq)∣ H₂(g)∣ Pt